P-Block Elements Short Notes: Download PDF, DPP and Online Test

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P-Block Elements (General Properties)

• Inert pair effect:
• Nature of oxide:
• Diagonal relationship
• Covalency
• Types of bonding

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Inert pair effect

The occurrence of oxidation states two unit less than the group oxidation states

Thus Tl⁺ is more stable in solution than Tl³⁺.

Thus Pb²⁺ is more stable in solution than Pb⁴⁺.

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Types and nature of oxides

Acidic oxide:     React with base

Basic oxide:      React with acid

Amphoteric oxide:   React with both acid and base

Neutral oxide: Neither reacts with acid nor with base

Diagonal relationship

Basis of Diagonal relationship:

Ionic size, charge to mass ratio and polarization power

Covalency

It is the number of covalent bonds it forms with other atoms.

It is due to the absence of d orbitals that the maximum covalence of B,C,N,O is 4.

tetrahedral [M(OH)₄]^– and octahedral [M(H₂O)₆]³⁺,

Types of Bonding

1.       C=C, C≡C, C=O, N≡N, C=N, C≡N, N=O).

2.      The heavier elements do form π bonds but this involves d orbitals (dπ–pπ or dπ –dπ).

3.      d orbitals are of higher energy than the p orbitals, they contribute less to the overall stability of molecules than does p π – p π   bonding.

Group-13 (Boron Family)

Gallium, melting point (303K), could exist in liquid state during summer. Boron high boiling point (2676K)

Atomic radius           Atomic radius of Ga is less than that of Al

Ionization enthalpy        B > Tl > Ga > Al > In

Electronegativity     B > Al < Ga < In < Tl

+1 oxidation state     B < Al < Ga < In < Tl

Boric acid (Orthoboric acid) (H₃BO₃)

Boric acid is a weak monobasic acid.

It is not a protonic acid but acts as a Lewis acid by accepting electrons from a hydroxyl ion

B(OH)₃ + 2H₂O → [B(OH)₄]^– + H₃O⁺

Orthoboric acid is used as a mild antiseptic.

H₃BO₃ → HBO₂ → B₂O₃

Group 14 Elements: Carbon Family

The dioxides

CO₂, SiO₂ and GeO₂ are acidic,

SnO₂ and PbO₂ are amphoteric in nature.

Monoxides

CO is neutral,

GeO is distinctly acidic whereas

SnO and PbO are amphoteric

+2 oxidation state increases in the sequence Ge < Sn < Pb

GeX₄ is more stable than GeX₂, whereas PbX₂ is more than PbX₄.

Except CCl₄, not hydrolysed by water because absence of d orbital.

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Catenation: Carbon atoms have the tendency to link with one another through covalent bonds to form chains and rings.

C  > >  Si  > Ge ≈ Sn

Lead (Pb) does not show catenation.

Allotropes of Carbon

Allotropy or allotropism is the property of some chemical elements to exist in two or more different forms, in the same physical state

1.       Two types crystalline as well as amorphous

2.      Diamond and graphite are two well-known crystalline forms of carbon.

3.      Amorphous: Coke, charcoal, carbon black

4.      Third form of carbon known as fullerenes

5.      Graphite is thermodynamically most stable allotrope of carbon and, therefore, Δf H^(-) of graphite is taken as zero.

Diamond

1.       Crystalline three dimensional lattice

2.      Each carbon atom undergoes sp³ hybridization (tetrahedral)

3.      The C–C bond length is 154 pm

4.      Hardest substance on the earth

5.      Bad conductor of electricity

6.      Highest thermal conductivity

7.       High refractive index

Graphite

1.       Layered structure, black, metallic luster

2.      Layers are held by van der Waals forces and distance between two layers is 340 pm.

3.      Each layer is composed of planar hexagonal rings of carbon atoms. C—C bond length within the layer is 141.5 pm.

4.      Each carbon atom sp2 hybridization (three sigma bonds)

5.      Fourth electron forms a π bond. The electrons are delocalized over the whole sheet.

6.      Good conductor of electricity (free mobile electrons)

7.       It is very soft and slippery

Fullerene (buckminsterfullerene)

1.       It’s a polygon, contains twenty six- membered rings and twelve five membered rings.

2.      A six membered ring is fused with six or five membered rings

3.      Five membered ring can only fuse with six membered rings.

4.      All the carbon atoms are sp2 hybridisation.

5.       Electron at each carbon is delocalised gives, aromatic character to molecule.

6.      Each carbon atom forms three sigma bonds with other three carbon atoms.

7.       Single and double bonds with C–C distances of 143.5 pm and 138.3 pm respectively.